Rates Equations

Question 1

Answer 1

G

Question 2

Answer 2

Question 3

Answer 3

Question 4

Answer 4

Question 5

rate = k[CH3COCH3][H+]

Answer 5

Question 6

Answer 6

Question 7

Answer 7

Question 8

1. Draw the structure of the product distilled off and give its name.
2. Give the formula of the product left in the distillation flask and give a use for it.

Answer 8

Question 9

State how the value of the rate constant, k, would change, if at all, if the concentration of A were increased in a series of experiments.

Answer 9

No change

Question 10

Answer 10

Power (or index or shown as x in [ ]) of concentration term
(in rate equation) (1)

Question 11

Answer 11

A - second order
B - zero order

Question 12

Answer 12

C

Question 13

How can you tell that H+ acts as a catalyst in this reaction?

Answer 13

Appears in the rate equation
Does not appear in the overall equation

Question 14

Answer 14

Question 15

The reaction is zero order with respect to B.
State the significance of this zero order for the mechanism of the reaction.
rate = k[a]^2

Answer 15

Slow step or rds involves only A OR
B does not appear in the slow step or the rds

Question 16

The rate equation for a reaction is
rate = K[E]
Explain qualitatively why doubling the temperature has a much greater effect on the rate of the reaction than doubling the concentration of E.

Answer 16

Reaction occurs when molecules have E>Ea
Doubling T by 10 °C causes many more molecules to have this E
Whereas doubling [E] only doubles the number with this E

Question 17

Answer 17

Question 18

Answer 18

B

Question 19

The experiment in part (i) is repeated at the same temperature but after the addition of extra solvent so that the total volume of the mixture is doubled.
Deduce the new initial rate of reaction.

Answer 19

8.3x10-6